A gas mixture is made by combining 7.0 g each of Ar, Ne, and an unknown diatomic gas. At STP, the mixture occupies a volume of 16.60 L. What is the molar mass of the unknown gas?

$P=(nRT)/(V)$........ And solve for $n=(PV)/(RT)$ $=$ $(86.11*atmxx1.500*L)/(0.0821*L*atm*K^-1*mol^-1xx298*K)$ $n=5.28*mol$ But $n=n_"He"+n_"unknown gas"$, i.e. $5.28*mol=(20*g)/(4*g*mol^-1)+n_"unknown gas"$ And thus $n_"unknown gas"=(5.28-5)*mol=0.280*mol$. And thus $"molecular mass of unknown gas"$ $=$ $(20*g)/(0.280*mol)=71.5*g*mol^-1$. And clearly,...

The molar mass of the gas is 38.0 g/mol. One way to solve this problem is to use the . $PV = nRT$ $n = m/M_"r"$, where $m$ is the...

The molar volume at $"STP"$ is $22.4*L*mol^-1$. Given this, if we divide the mass by the molar quantity of the gas we get an answer in $g*mol^-1$ as required: $(1.00*L)/(22.4*L*mol^-1)$...

We use the Ideal Gas Equation....... $PV=nRT$ And thus $n="Mass"/"Molar Mass"=(PV)/(RT)$ And so, $"Molar Mass"=("Mass"xxRT)/(PV)$ $=(0.20*gxx0.0821*cancelL*cancel(atm)*cancel(K^-1)*mol^-1xx300*cancelK)/(1*cancel(atm)xx0.200*cancelL)$ $=24.6*g*mol^-1$. I think this is dimensionally correct, however, it does not correspond to a...

Depending on your syllabus, at $"STP"$ $1*mol$ of Ideal Gas occupies $22.4*dm^3$, i.e. $22.4*dm^3*mol^-1$.......and note that $1*dm^3=1xx(10^-1*m)^3=1/1000*m^3=1*L$, cos' there are $1000*L$ in a $"cubic metre"$. And thus the $"molar mass"="mass"/"molar...

Use the ideal gas equation $P.V=n.R.T$ $P.V= m/(MM).R.T$ $P.MM= m/V.R.T$ $P.MM= d.R.T$ $P" is the pressure of the gas (" atm")"$ $MM" is the molar mass ("g.mol^-1")"$ $d" is the...

STP is defined as 1 bar and 0 °C. The molar volume at STP is 22.71 L/mol. $"Moles of Ne" = 36.2 color(red)(cancel(color(black)("g Ne"))) × "1 mol Ne"/(20.18 color(red)(cancel(color(black)("g...

So neon occupies 33.6 g First we find the number of moles of Ne= $(mass)/"molar mass"$ No. of moles= $(33.6)/"20"$ No. of moles= 1.68 mol Then, we can find volume...

The first thing to do here is use the molar masses of the two to determine how many moles of each you have present in your sample. $3.54...

The first thing to do is write out what the STP conditions are Pressure - $"100 kPa"$ Temperature - $0^@"C"$ SInce no mention about the number...